Chemistry

Q: The following four spheres represent an Mg atom, an Mg2+ ion, a S atom, and a S2- ion, not necessarily in that order. Use your knowledge about the relative sizes of atoms, cations, and anions to determine which of the following sets of reactions is most consistent with the sizes of the atoms and ions shown below.A) A -> B + 2e- and C -> D + 2e-B) A -> B + 2e- and D -> C + 2e-C) B -> A + 2e- and C -> D + 2e-D) B -> A + 2e- and D -> C + 2e-

Q: The following four spheres represent a Na atom, a Na+ ion, a Cl atom, and a Cl- ion, not necessarily in that order. Use your knowledge about the relative sizes of atoms, cations, and anions to determine which of the following sets of reactions is most consistent with the sizes of the atoms and ions shown below.A) A -> B + e- and C -> D + e-B) A -> B + e- and D -> C + e-C) B -> A + e- and C -> D + e-D) B -> A + e- and D -> C + e-

Q: Which sphere represents the monatomic cation? A) A B) B C) C D) D

Q: Which sphere represents the monatomic anion? A) A B) B C) C D) D

Q: Which sphere represents the nonmetal atom? A) A B) B C) C D) D

Q: Which sphere represents the metal atom? A) A B) B C) C D) D

Q: Atoms of which element, indicated by letter on the periodic table, is expected to have the smallest atomic radius? A) A B) B C) C D) D

Q: Atoms of which element, indicated by letter on the periodic table, are expected to have the largest atomic radius? A) A B) B C) C D) D

Q: Which element, indicated by letter on the periodic table above, has a 3+ ion with the electron configuration 1s2 2s2 2p6 3s2 3p6? A) A B) B C) C D) D

Q: Which element, indicated by letter on the periodic table above, has a 3+ ion with the electron configuration [Kr]4d5? A) A B) B C) C D) D

Q: Which element, indicated by letter on the periodic table above, has a 1+ ion with the electron configuration [Xe]6s2 4f14 5d10? A) A B) B C) C D) D

Q: Which element, indicated by letter on the periodic table above, has a 2+ ion with the electron configuration [Ar]3d10? A) A B) B C) C D) D

Q: Which statement is inconsistent with the chemistry of the noble gases? A) Both helium and radon are radioactive. B) Helium and neon are both lighter than air. C) Neon and argon are used in decorative or designer lights. D) Xenon and krypton react with fluorine to form fluorides.

Q: Which of the following statements about helium is inconsistent with its chemistry? A) A helium oxygen mixture is used as a deep-sea diving gas instead of compressed air. B) In its liquid form it is used as a cryogenic coolant for superconductors. C) It is one of the more reactive elements of its group. D) Its melting point is -272.2C and its boiling point is -268.9C.

Q: Predict the product(s) of the reaction of Br2(aq) with I-(aq). A) No reaction B) IBr3-(aq) C) BrO3-(aq) and I2(aq) D) Br-(aq) and I2(aq)

Q: Interhalogen compounds can be produced by reacting two different halogens together. Which one of the following compounds does not exist? A) ClF B) ClBr C) ClBr3 D) IF3

Q: Which of the following reactions is inconsistent with the chemistry of the halogens?A) H2(g) + Cl2(g) -> 2 HCl(g)B) Fe(s) + F2(g) -> FeF2(s)C) Br2(l) + 2 Cl-(aq) -> 2 Br-(aq) + Cl2(g)D) I2(s) + 3 Cl2(g) -> 2 ICl3(s)

Q: Which of the hydrogen halide acids is used to etch glass? A) HF B) HCl C) HBr D) HI

Q: Metals tend to react with the halogens to form metal halides. What is the reactivity order for the halogens? A) F2 > Cl2 > Br2 > I2 B) Cl2 > F2 > Br2 > I2 C) Br2 > I2 > Cl2 > F2 D) I2 > Br2 > Cl2 > F2

Q: Both chlorine and bromine can be produced in the laboratory by reacting the halides with manganese(IV) oxide. If the following equation is balanced in an acidic solution, then the MnO2 is acting as a(n) ________ and the coefficient in front of H+ is ________.____ MnO2(s) + ____ Cl-(aq) + ____ H+(aq) -> ____ Mn2+(aq) + ____ Cl2(g) + ____ H2O(l)A) oxidizing agent, 2B) oxidizing agent, 3C) oxidizing agent, 4D) reducing agent, 3

Q: Which group of elements are found as diatomic molecules? A) alkali metals B) alkaline earth metals C) halogens D) noble gases

Q: Which of the following elements is a solid at room temperature? A) fluorine B) chlorine C) bromine D) iodine

Q: Which of the following elements is a liquid at room temperature? A) fluorine B) chlorine C) bromine D) iodine

Q: Predict the product(s) when the reactants Be(s) + Br2(l) are mixed. A) BeBr(s) B) BeBr2(s) C) Be2Br(s) D) BeBr3(s)

Q: Calcium, strontium, and barium are all prepared commercially by the same method which is A) electrolysis of the molten metal oxides. B) electrolysis of the molten metal halides. C) chemical reduction of the metal oxides with aluminium. D) chemical reduction of the metal halides with oxygen.

Q: Group 2A metals tend to be somewhat less reactive than alkali metals, and the order of their reactivity is A) Ba > Sr > Ca > Mg > Be. B) Be > Mg > Ca > Sr > Ba. C) Ca > Mg > Be > Ba > Sr. D) Sr > Ca > Mg > Be > Ba.

Q: Which alkaline earth metal reacts the most vigorously with water at room temperature? A) Be B) Ca C) Ba D) Sr

Q: Which is not generally considered to be a chemical reaction of the alkaline earth metal magnesium?A) 2 Mg(g) + O2(g) -> 2 MgO(s) at room temperatureB) 3 Mg(s) + N2(g) -> Mg3N2(s) at elevated temperaturesC) Mg(s) + 2 H2O(l) -> Mg(OH)2(s) + H2(g) at room temperatureD) Mg(s) + F2(g) -> MgF2(s) at room temperature

Q: Which is not generally considered to be a chemical reaction of the alkaline earth metal calcium?A) Ca(s) + Cl2(g) -> CaCl2(s)B) 2 Ca(s) + 2 H2O(l) ->2 Ca(OH)2(aq) + H2(g)C) 6 Ca(s) + 2 N2(g) -> 2 Ca3N2(s)D) Ca(s) + O2(g) -> CaO2(s)

Q: An incorrect statement about the alkaline earth metals is: A) Melting points generally decrease as one descends the group. B) Densities are less than those of the corresponding alkali elements of the same period. C) Ionic radii of the M2+ ion increases as one descends the group. D) The first ionization energy is less than that of the second ionization energy.

Q: The alkali metals K, Rb, and Cs are commercially produced by A) chemical reduction of their molten salts. B) electrolysis of their molten salts. C) thermal decomposition of their molten metal halides. D) thermal decomposition of their molten metal oxides.

Q: The alkali metals Li and Na are commercially produced by A) chemical reduction of their molten salts. B) electrolysis of their molten salts. C) thermal decomposition of their molten metal halides. D) thermal decomposition of their molten metal oxides.

Q: Which alkali metal reacts with nitrogen to form a nitride? A) Li B) Na C) K D) All of these

Q: Which is not a chemical reaction of the alkali metal potassium?A) K(s) + O2(g) -> KO2(s)B) 2 K(s) + 2 H2O(l) -> 2 KOH(aq) + H2(g)C) 2 K(s) + H2(g)-> 2 KH(s)D) 6 K(s) + N2(g) -> 2 K3N(s)

Q: Which is not a chemical reaction of the alkali metal sodium?A) 4 Na(s) + 2 O2(g) -> 2 Na2O(s) + Na2O2(s)B) 2 Na(s) + 2 NH3(l) ->2 NaNH2(sol) + H2(g)C) 2 Na(s) + Cl2(g) -> 2 NaCl(s)D) 2 Na(s) + 2 H2O(l) -> 2 NaOH(aq) + H2(g)

Q: Which alkali metal forms preferentially a peroxide and superoxide? A) Li B) Na C) K D) Mg

Q: Which alkali metal forms preferentially an oxide rather than a peroxide or superoxide? A) Li B) Na C) K D) Rb

Q: Which ionic compound would be expected to have the highest lattice energy? A) Li2O B) Na2O2 C) KO2 D) RbO2

Q: Which ionic compound would be expected to have the highest lattice energy? A) NaCl B) MgO C) AlF3 D) Al2O3

Q: Which ionic compound would be expected to have the highest lattice energy? A) Na2O B) MgO C) Al2O3 D) CO2

Q: Which of the following ionic compounds would be expected to have the highest lattice energy? A) LiCl B) NaCl C) KCl D) RbCl

Q: Which of the following ionic compounds would be expected to have the highest lattice energy? A) NaF B) NaCl C) NaBr D) NaI

Q: Which chemical process is associated with the lattice energy for sodium chloride?A) NaCl(s) -> Na+(g) + Cl-(g)B) NaCl(g) -> Na+(g) + Cl-(g)C) Na(s) + 1/2 Cl2(g) ->NaCl(s)D) NaCl(s) + H2O(l) -> Na+(aq) + Cl-(aq)

Q: Calculate the electron affinity for the formation of the hydride ion from the following information: A) -50.1 kJ/mol B) -70.1 kJ/mol C) -816 kJ/mol D) -1632 kJ/mol

Q: Calculate the energy change for the formation of MgBr2(s) from its elements in their standard states: A) -150.8 kJ/mol B) -286.0 kJ/mol C) -499.2 kJ/mol D) -5682 kJ/mol

Q: Calculate the energy change in kJ/mol for the reaction Li+(g) + F-(g) -> Li(g) + F(g) using the following information:Li(g) -> Li+(g) + e- +520 kJ/molF(g) + e- -> F-(g) -328 kJ/molA) -848 kJ/molB) -192 kJ/molC) +192 kJ/molD) +848 kJ/mol

Q: Calculate the lattice energy for MgO(s) using a Born-Haber cycle and the following information: A) +1842 kJ/mol B) +2444 kJ/mol C) +3844 kJ/mol D) +4108 kJ/mol

Q: Calculate the energy change for the formation of CaF2(s) from its elements in their standard states and the following information: A) +4046 kJ/mol B) -965 kJ/mol C) -1214 kJ/mol D) -3286 kJ/mol

Q: Calculate the lattice energy for MgCl2(s) using a Born-Haber cycle and the following information: A) +641.6 kJ/mol B) +1240.5 kJ/mol C) +1882.1 kJ/mol D) +2523.7 kJ/mol

Q: Calculate the lattice energy for NaCl(s) using a Born-Haber cycle and the following information: A) +34.8 kJ/mol B) +690.3 kJ/mol C) +787.2 kJ/mol D) +1512 kJ/mol

Q: Calculate the energy change for the formation of LiCl(s) from its elements in their standard states and the following tabulated information: A) +1305.7 kJ/mol B) +296.9 kJ/mol C) -400.3 kJ/mol D) -627.2 kJ/mol

Q: In the reaction of sodium metal with chlorine gas which of the following processes releases energy?A) Cl2(g) -> 2 Cl(g)B) Cl(g) + e- -> Cl-(g)C) Na(s) -> Na(g)D) Na(g) -> Na+(g) + e-

Q: The octet rule is most likely to fail occasionally for which of the following elements? A) C B) N C) Na D) S

Q: How many electrons does magnesium lose and nitrogen need to form Mg3N2? A) magnesium loses 2 and nitrogen gains 2 B) magnesium loses 2 and nitrogen gains 3 C) magnesium loses 3 and nitrogen gains 2 D) magnesium loses 3 and nitrogen gains 3

Q: An element M reacts with chlorine to form MCl2, with oxygen to form MO, and with nitrogen to form M3N2. The most likely candidate for the element is A) Li B) Mg C) Al D) Si

Q: Which species does not have an octet of electrons for its outer core? A) C4- B) P3- C) O2- D) Mg+

Q: To reach a noble gas electron configuration how many electrons would sulfur have to adopt? A) 1 B) 2 C) 6 D) 8

Q: An element that has the valence electron configuration 3s23p3 belongs to which period and group? A) period 3; group 3A B) period 3; group 5A C) period 4; group 3A D) period 4; group 5A

Q: How many valence shell electrons does an atom of aluminum have? A) 1 B) 2 C) 3 D) 13

Q: What is the general trend in ionization energy and electron affinity values? A) Both decrease as one traverses a period from left to right and both decrease as one descends a group. B) Both decrease as one traverses a period from left to right and both increase as one descends a group. C) Both increase as one traverses a period from left to right and both decrease as one descends a group. D) Both increase as one traverses a period from left to right and both increase as one descends a group.

Q: Which of these elements has the most favorable (most negative) electron affinity? A) Ca B) N C) Ne D) S

Q: Which element has the least favorable (least negative) electron affinity? A) B B) C C) N D) O

Q: Which element has the most favorable (most negative) electron affinity? A) Na B) Mg C) O D) Ne

Q: Which element has the most favorable (most negative) electron affinity? A) B B) C C) Li D) N

Q: Which electron affinity process would liberate the most energy?A) [He] 2s2 + e- ->[He] 2s2 2p1B) [He] 2s2 2p2 + e- -> [He] 2s2 2p3C) [He] 2s2 2p3 + e- -> [He] 2s2 2p4D) [He] 2s2 2p6 + e- -> [He] 2s2 2p6 3s1

Q: Which liberates the most energy?A) Br(g) + e- -> Br-(g)B) Cl(g) + e- -> Cl-(g)C) F(g) + e- -> F-(g)D) I(g) ->I-(g)

Q: Which liberates the most energy?A) Li(g) + e- -> Li-(g)B) Na(g) + e- -> Na-(g)C) K(g) + e- -> K-(g)D) Rb(g) + e- -> Rb-(g)

Q: Which period 2 element has successive first through seventh ionization energies (kJ/mol) of Ei1 = 1,402; Ei2 =2,856; Ei3 =4,578; Ei4 =7,475; Ei5 =9,445; Ei6 =53,267; and Ei7 = 64,360? A) B B) C C) N D) O

Q: Which period 3 element has successive first through seventh ionization energies (kJ/mol) of Ei1 = 578; Ei2 = 1,817; Ei3 = 2,745; Ei4 = 11,575; Ei5 = 14,830; Ei6 = 18,376; and Ei7 = 23,293? A) Mg B) Al C) S D) Cl

Q: Consider the following electron configurations for neutral atoms: atom I = 1s22s22p63s2 atom II = 1s22s22p63s23p4 atom III = 1s22s22p63s23p6 Which atom would be expected to have the largest third ionization energy? A) atom I B) atom II C) atom III D) All of these atoms would be expected to have the same third ionization energy.

Q: Which of the following represents the change in electronic configuration that is associated with the first ionization energy of magnesium?A) [Ne]3s13p1 -> [Ne]3s1 + e-B) [Ne]3s2 -> [Ne]3s13p1C) [Ne]3s2 -> [Ne]3s1 + e-D) [Ne]3s2 + e- -> [Ne]3s23p1

Q: Which of the following atoms with the specified electronic configurations would have the lowest first ionization energy? A) [He]2s22p3 B) [Ne]3s23p4 C) [Xe]6s1 D) [Xe]6s24f145d106p1

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